What intermolecular forces are important for the molecule below?[Check all that apply.]HN,CH3O lon-DipoleHydrogen BondingDipole-DipoleLondon Dispersion ForcesO None of these

Intermolecular forces are divided in many categories such as hydrogen bonding, dipole-dipole…

Answered: What intermolecular forces are…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter8: Molecules And Materials

Section: Chapter Questions

Problem 8.37PAE: 8.37 If a molecule is not very polarizable, how will it respond to an external electric field?

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Similar questions

Pick all of the molecules with a permanent net electric dipole : CHCl3, I2
Identify what type of intermolecular forces exist between the following pairs. ( I already anwer it but I am not sure with my answers Please check my answer and correct it if it wrong. Thank you!) HBr and H₂S Answer: Dipole-dipole Cl₂ and CBr₄ Answer: London dispersion forces I₂ and NO₃¹⁻ Answer: Dipole-induced dipole NH₃ and C₆H₆ Answer: Ion- induced dipole
Examine the elements in the second row of the periodic table. Note that HF, H2O, NH3 and CH4 are sp3 hybridized. The first three are all capable of hydrogen bonding. Methane, however, is not capable of hydrogen bonding. Explain.
the strongest IMF present between molecules of each compound. CS2 [ Choose ] dipole-dipole hydrogen bonding dispersion forces ion-ion CH2O [ Choose ] dipole-dipole hydrogen bonding dispersion forces ion-ion HF [ Choose ] dipole-dipole hydrogen bonding dispersion forces ion-ion MgF2 [ Choose ] dipole-dipole hydrogen bonding dispersion forces ion-ion
Attraction between atoms to weak. 1. How would you describe the spacing between the atoms? Are the atoms free to move around? 2. What is the likely phase (solid, liquid, or gas) of the substance that is comprised of the atoms you have just described.
Which molecule(s) will experience the Hydrogen Bonding force? Select all that apply. Group of answer choices: A) H2O B) NH3 C) H2 D) N2
TRUE OR FALSE 1. molecules with temporary dipole moment tend to align with opposite polarities in the solid phase for maximum attractive attraction. 2.the boiling point of compounds containing elements in the same periodic group is inversely proportional to the elements molar mass. 3.when adhesion is greater than cohesion, a convex appearance of the liquid in a tube is evident. 4.when cohesion is greater than adhesion, a concave appearance of the liquid in tube is evident.
Answer each question and justify your answer by doing ALL of the following: • Identify the type of substance and important interparticle force(s) for both substances. − Explain how you know (substances and forces). − For each molecular substance, fully justify how you know if it is polar or nonpolar. Provide a Lewis structure, a geometry sketch, calculation of |ΔEN| values, and a discussion of symmetry. • Identify which of the two substances has stronger interparticle forces. If they have the same type of interparticle force, explain how you know which is stronger. • Answer the question by connecting the property asked about to strength of interparticle forces. • Use complete sentences, write all words out (no abbreviations) and be specific and complete with all explanations. Do not refer to any actual data. 10-3. Does CH4O or CH3F have the higher boiling point? 10-5. Does BaSO4 or KCN have the lower melting point?
Which compound(s) exhibit(s) dipole-dipole forces? (hint: draw the lewis structures) 1. BCl3 3. NF3 2. XeF2 4. OCl2 a. 3 only b. 2, 3, and 4 c. 1 and 2 d. 3 and 4
What is the strongest interparticle force in each of the following substances?a) CH3Clhydrogen bondingdipole―dipoledispersion(b) CH3CH3dipole―dipoledispersionhydrogen bondingc) NH3hydrogen bondingdispersiondipole―dipole
The table below shows some physical properties of halogenatedliquids.Which of the following statements best explains these data?(a) The larger the dipole moment, the stronger the intermolecularforces, and therefore the boiling point is lowest for themolecule with the largest dipole moment. (b) The dispersionforces increase from F to Cl to Br; since the boiling point alsoincreases in this order, the dispersion forces must make a fargreater contribution to intermolecular interactions thandipole–dipole interactions. (c) The trend in electronegativityis F 7 Cl 7 Br; therefore, the most ionic compound 1CH2F22has the lowest boiling point, and the most covalent compound1CH2Br22 has the highest boiling point. (d) Boiling point increaseswith molecular weight for these nonpolar compounds.
The table below shows some physical properties of halogenatedliquids. Which of the following statements best explains these data?(a) The larger the dipole moment, the stronger the intermolecularforces, and therefore the boiling point is lowest for themolecule with the largest dipole moment. (b) The dispersionforces increase from F to Cl to Br; since the boiling point alsoincreases in this order, the dispersion forces must make a fargreater contribution to intermolecular interactions thandipole-dipole interactions. (c) The trend in electronegativityis F > Cl > Br; therefore, the most ionic compound (CH2F2)has the lowest boiling point, and the most covalent compound(CH2Br2) has the highest boiling point. (d) Boiling point increaseswith molecular weight for these nonpolar compounds.

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What intermolecular forces are important for the molecule below? [Check all that apply.] HN CH3 O lon-Dipole Hydrogen Bonding Dipole-Dipole O London Dispersion Forces None of these